The van der Waals forces in halogen decrease in the order (a) I2>Br2>Cl2>F2 (b) F2>Cl2>Br2>I2 (c

step 1 explanation for the given question here we have problem 71 that is the wonderful forces in halog

The van der Waals forces in halogen decrease in the order...

The van der Waals forces in halogen decrease in the order (a) $\mathrm{I}_{2}>\mathrm{Br}_{2}>\mathrm{Cl}_{2}>\mathrm{F}_{2}$ (b) $\mathrm{F}_{2}>\mathrm{Cl}_{2}>\mathrm{Br}_{2}>\mathrm{I}_{2}$ (c) $\mathrm{I}_{2}>\mathrm{F}_{2}>\mathrm{Br}_{2}>\mathrm{Cl}_{2}$ (d) $\mathrm{Cl}_{2}>\mathrm{I}_{2}>\mathrm{Br}_{2}>\mathrm{F}_{2}^{2}$

The van der Waals forces in halogen decrease in the order
(a) $\mathrm{I}_{2}>\mathrm{Br}_{2}>\mathrm{Cl}_{2}>\mathrm{F}_{2}$
(b) $\mathrm{F}_{2}>\mathrm{Cl}_{2}>\mathrm{Br}_{2}>\mathrm{I}_{2}$
(c) $\mathrm{I}_{2}>\mathrm{F}_{2}>\mathrm{Br}_{2}>\mathrm{Cl}_{2}$
(d) $\mathrm{Cl}_{2}>\mathrm{I}_{2}>\mathrm{Br}_{2}>\mathrm{F}_{2}^{2}$

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Key Concepts

Molecular Size and Mass

The size and mass of a molecule or atom are directly related to its polarizability and the strength of its London dispersion forces. Larger, heavier molecules generally have more electrons and a more easily disturbed electron cloud, thus experiencing stronger van der Waals forces compared to smaller, lighter molecules.

Polarizability

This refers to the ease with which the electron cloud around an atom or molecule can be distorted, thereby forming temporary dipoles. Higher polarizability leads to stronger dispersion forces, which is why larger or heavier atoms tend to exhibit stronger van der Waals interactions.

Van der Waals Forces

These are weak intermolecular attractions that occur between molecules, atoms, and ions. They include various types of forces such as dispersion forces, dipole-dipole interactions, and sometimes hydrogen bonds. In nonpolar molecules, van der Waals forces are primarily due to instantaneous dipoles that induce further dipoles in adjacent molecules.

London Dispersion Forces

A subtype of van der Waals forces, London dispersion forces arise from temporary fluctuations in electron density which create transient dipoles. They are especially significant in nonpolar molecules and larger atoms, where increased electron count enhances the strength of these forces.

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